The following mechanism for the gas phase decomposition of oxygen difluoride is consistent with the observed rate law. step 1 fast: 2 OF2=0;F4 step 2 slow: 0,F4¬0; +2 F; (1) What is the cquation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"|B]". , where 'I' is understood (so don't write it if it's a 'l') for m, n etc.

The following mechanism for the gas phase decomposition of oxygen difluoride is consistent with the observed rate law. step 1 fast: 2 OF2=0;F4 step 2 slow: 0,F4¬0; +2 F; (1) What is the cquation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"|B]". , where 'I' is understood (so don't write it if it's a 'l') for m, n etc.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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2. Consider the kinetic data of the reaction of P + 2 Q + 2+ - PQ, + Z*and answer the succeeding questions: Experiment P (M) Q (M) Temp ("C) Initial Rate, M/s 1 0.01150 0.01200 0.00000 25 4.80 x 10-4 2 0.02300 0.01200 0.00000 25 1.92 x 10-3 3 0.01150 0.02400 0.00000 25 9.60 x 10-4 4 0.04600 0.01200 0.00000 25 7.68 x 10-3 5 0.01150 0.04800 0.00000 25 1.92 x 10-3 6 0.01150 0.01200 0.00000 10 5.10 x 10-5 0.01150 0.01200 0.00000 40 4.55 x 10-3 0.01150 0.01200 0.00500 10 4.98 x 10-5 0.01150 0.01200 0.01050 25 4.82 x 104 10 0.01150 0.01200 0.02100 40 4.44 x 10-3 A. Determine the rate order with respect to P. Determine the rate order with respect to Q. C. Determine the rate law of the reaction. What is the average rate constant? Indicate the appropriate units. E. What is the energy of activation and frequency factor of the reaction without the additive ion? Include the equation of the best fit line of the Arrhenius equation and RSQ Note: Use the calculated rate constant in set up 1 for 25°C…
For an autocatalytic reaction : A → B + …… where -d[A]/dt = k[A][B]. Assume that [B]o ≠0 Letting [A] = Ao – x and [B] = Bo +x -d[A]/dt = -d[Ao -x]/dt = dx/dt and dx/dt = k[Ao- x] [Bo + x] Show that [B] = {[A]o + [B]o } / [Ao/Bo] exp{- [A]o + [B]0 }kt + 1
For a reaction A products, sicessive half_For a reaction A→ products, successive half-lives are observed to be 10.0,20.0 and 40.0 min for an experiment in which the initial concentration of A=0.10M. Calculate the concentration of A(M) after 39.37 minutes. Report your answer to 4 significant fgures.
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H,(g) + 2 NO(g) → N,0(g) + H,0(g) k1 2 H2(9) + N,0(9) → N2(9) + H,O(g) Suppose also k, «k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k U Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k-2 for k = the reverse of the two elementary reactions in the mechanism.
Concentration-Time Relationships (See Section 15.4 and Examples 15.5-15.7.) 15. The rate equation for the hydrolysis of sucrose to fruc- tose and glucose CRH2O1(aq) + H¿O(€) → 2 C,H12O6(aq) is -A[sucrose]/At = k[C¡2H2O1]. After 27 minutes %3D at 27 °C, the sucrose concentration decreased from 0.0146 M to 0.0132 M. Find the rate constant, k.
4. The following data were obtained for the follwing chemical reaction: 2A + 3B ---> 2C + D Initial [A] Initial [B] Initial Rate of Formation Trial # (mmol/L) (mmol/L) of D (mmol/L*s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (b) Find the rate constant, k, with units.
Give typing answer with explanation and conclusion
A reaction is described as follows: k1 X + Y The table below shown the initial rates of the formation of product Z (Vo) for various reactant concentrations. From the data given, answer the followings: [X], mol L- [Y], mol L-1 34 Vo (x 103 mol L-s') 22 1.00 70 45 4.20 8.08 71 89 (i) The rate law of formation of product Z, (ii) The overall rate order and the order with respect to each component, and (iii) The rate constant (state clearly its units and coefficients).
For the gas phase decomposition of ethyl acetate, CH;COOC,H,–CH,COOH + C2H4 the rate constant has been determined at several temperatures. When In k -1 in s is plotted against the reciprocal of the Kelvin temperature, the resulting linear plot has a slope of -2.41x10* K and a y-intercept of 28.8. The activation energy for the gas phase decomposition of ethyl acetate is kJ/mol.
The following data were obtained for the reaction 2C102 (ag) + 20H (ag) → Cl0; (ag) + C102 (ag) + H,0(1) A[CIO2] where Rate = - At [C102]o (mol L) [OH ], (mol L) Initial Rate (molL·s) 0.0750 0.150 1.94 x 10-1 0.150 0.150 7.76 x 10-1 0.150 0.0750 3.88 x 10-1 a Determine the rate law. (Use k for the rate constant.) Rate = k[ClO,][OH] b Determine the value of the rate constant. Rate constant = 2.30x1 / L²/mol? - s c What would be the initial rate for an experiment with [CIO2], = 0.140 mol/L and [OH], = 0.0668 mol/L? Rate = mol/L·s
A reiction is described as follows: 2A (g) + 2B (g) -+C (g) Exp. (A). M Initial rate (x10* Ms') 0.15 0.15 0.15 1.24 2.46 4.95 2. 032 0.15 3 0.30 From the data given above, determine the followings: (1) The rate law formula in terms of formation of product C, (ii) The overall order and the order with respect to each component, (ii) The rate constant (state clearly its units and coefficients), (iv) Find the rate of reaction when (A] - [BI =0.20 M.
tab esc slock ||| = OKINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism with an initi.... Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) + O₂ (g). -NO₂(g) + O₂(g) k₁ 2 NO₂ (g) + NO₂ (g) → N₂O5 (g) k₂ Suppose also k₁ «k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. BE 1 Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Explanation Q A @ 2 Check W S X # 3 E 0 rate = k 14 D $ 4 rate constant > R F % 5 © Stv T MacBook Pro 6 G We Y & 7 H 0-0 U 00 Ⓒ2022 McGraw Hill LLC. All R You * 00 00 8 S a (